1. This lab calls for you to titrate 1.00 mL of 3.00% H2O2 using the reaction below.

   5H2O2 + 2MnO4- + 6H+ 5O2 + 2Mn2+ + 8H2O

1. Assuming the density of the H2O2 is 1.00 g/mL, what mass of H2O2 is in your 1.00 mL sample?

2. How many moles is this?

3. Based on the stoichiometry of the reaction between MnO4- ions and H2O2 in acidic solution, estimate the volume of 0.020 M MnO4- solution required to titrate this 1.00 mL sample.

4. What is the maximum volume of H2O2 you can react with a full burette (50.0 mL) of KMnO4?

5. According to the equation above, what other substance do you need for this titration besides the KMnO4 and H2O2?

6. How many moles of this substance do you need for it to be in excess?

7. How many mL of a 3 M solution of this substance is necessary?